A Textbook of Physical Chemistry: Thermodynamics And Chemical Equilibrium (SI Unit), 5e, Volume 2

Title
Contents
1. Introduction to Thermodynamics
	1.1 Scope of Thermodynamics
	1.2 Basic Definitions
	1.3 Mathematical Background
	1.4 I UPAC Conventions of Work and Heat
	1.5 W ork Involved in Expansion and Compression Processes
	1.6 Reversible and Irreversible Processes
2. Zeroth and First Laws of Thermodynamics
	2.1 Zeroth Law of Thermodynamics
	2.2 First Law of Thermodynamics
	2.3 Mathematical Proof of Heat and Work Being Inexact Functions
	2.4 Change in Energy Function with Temperature
	2.5 E nthalpy Function
	2.6 Relation Between Heat Capacities
	2.7 Joule’s Experiment
	2.8 Joule-Thomson Experiment
	2.9 Joule-Thomson Coefficient and Van Der Waals Equation of State
	2.10 Thermodynamic Changes in Isothermal Variation in Volume of an Ideal Gas
	2.11 Thermodynamic Changes in Adiabatic Variation in Volume of an Ideal Gas
	2.12 Comparison Between Reversible Isothermal and Adiabatic Expansions of an Ideal Gas
	2.13 Thermodynamic Changes in Isothermal Variation in Volume of a Van Der Waals Gas
	2.14 Thermodynamic Changes in Adiabatic Variation in Volume of a Van Der Waals Gas
	2.15 Miscellaneous Numericals
3. Thermochemistry
	3.1 Scope of Thermochemistry
	3.2 E nthalpy of a Substance
	3.3 Change in Enthalpy During the Progress of a Reaction
	3.4 E nthalpy of Reaction
	3.5 E xothermic and Endothermic Nature of A Reaction
	3.6 I upac Recommendation of Writing Chemical Equation and Definition of Enthalpy of Reaction
	3.7 E nthalpy of Formation
	3.8 H ess’s Law of Constant Heat Summation
	3.9 Various Types of Enthalpies of Reactions
	3.10 Bond Enthalpies
	3.11 Variation in Enthalpy of A Reaction with Temperature (Kirchhoff’s Relation)
	3.12 Relation Between Energy and Enthalpy of a Reaction
	3.13 Adiabatic Flame Temperature
4. Se cond Law of Thermodynamics
	4.1 Necessity of the Second Law
	4.2 Carnot Cycle
	4.3 Expression for the Efficiency of a Carnot Cycle Involving Ideal Gas as a Working Substance
	4.4 Two Statements of Second Law of Thermodynamics
	4.5 Efficiency of the Carnot Cycle is Independent of the Working Substance
	4.6 Comparison of Efficiencies of Reversible and Irreversible Cyclic Processes
	4.7 The Thermodynamic or Kelvin Temperature Scale
	4.8 I dentity of Thermodynamic Scale with Ideal Gas Temperature Scale
	4.9 Definition of the Entropy Function
	4.10 The Value of dq (irr)/T for an Irreversible Cyclic Process
	4.11 The Clausius Inequality
	4.12 State Function Entropy From First Law of Thermodynamics
	4.13 Characteristics of The Entropy Function
	4.14 E ntropy as a Function of Temperature and Volume
	4.15 E ntropy as a Function of Temperature and Pressure
	4.16 E ntropy Changes for an Ideal Gas
	4.17 A Few Derivations Involving a Van Der Waals Gas
	4.18 Standard State for Entropy of an Ideal Gas
	4.19 E ntropy and Disorderliness
	4.20 E ntropy Change in Isothermal Expansion or Compression of an Ideal Gas
	4.21 E ntropy Change in Adiabatic Expansion or Compression of an Ideal Gas
	4.22 E ntropy Changes in a Few Typical Cases
	4.23 The Third Law of Thermodynamics
	4.24 E ntropy of Reaction and its Temperature and Pressure Dependence
	4.25 E ntropy and Probability
	4.26 Miscellaneous Numericals
5. Equilibrium Criteria, A and G Functions
	5.1 Criteria for Equilibrium Under Different Conditions
	5.2 Relation Between DG and DStotal for an Isothermal and Isobaric Processes
	5.3 Gibbs Free-Energy Change of A Chemical Equation
	5.4 Thermodynamic Relations Involving Functions A and G
	5.5 Relationship Between DrG° and Dr A°
	5.6 Pressure Dependence of Free Energy
	5.7 Fugacity Function and Its Determination for Real Gases
	5.8 Temperature Dependence of Free Energy
	5.9 Resume Concerning U, H, S, A and G
	5.10 Derivations of Some Thermodynamic Relations
	5.11 Bridgman Formulae to Write the Expressions of First Partial Derivatives
	5.12 Miscellaneous Numericals
6. S ystems of Variable Composition
	6.1 Partial Molar Quantities
	6.2 E xperimental Determination of Partial Molar Volumes
	6.3 Chemical Potential
	6.4 E xpressions of dU, dH, dA and dG for Multicomponent Open System
	6.5 Thermodynamic Relations Involving Partial Molar Quantities
	6.6 The Escaping Tendency
	6.7 Chemical Potential of a Gas
	6.8 Chemical Potential of a Gas in a Mixture of Ideal Gases
	6.9 Partial Molar Quantities of a Gas in a Mixture of Ideal Gases
	6.10 Additivity Rules
	6.11 Gibbs-Duhem Equation
7. The rmodynamics of Chemical Reactions
	7.1 Description of a Reaction in Progress
	7.2 Thermodynamics of Chemical Reactions (Reaction Potential)
	7.3 H omogeneous Ideal Gas Reaction
	7.4 E xpression of K p °for a Reaction Involving Heterogeneous Phases
	7.5 Dynamic Equilibrium (Law of Mass Action)
	7.6 General Rules to Write Q°and K ° p p for any Reaction
	7.7 Standard Equilibrium Constant in Units Other Than Partial Pressures
	7.8 Principle of Le Chatelier and Braun
	7.9 Temperature Dependence of Standard Equilibrium Constant P K°
	7.10 Pressure Dependence of Equilibrium Constants
	7.11 E ffect of an Inert Gas on Equilibrium
	7.12 General Treatment of a Reaction in Progress
	7.13 Characteristics of Homogeneous Gaseous Reactions
	7.14 Study of a Few Important Homogeneous Gaseous Reactions
	7.15 Miscellaneous Numericals
		Annexure Chemical Equilibrium in an Ideal Solution
Appendix I Values of Thermodynamic Properties
Appendix II Units and Conversion Factors
Index